OFFICIAL SYLLABUS

Unit I: Some Basic Concepts of Chemistry

(i) Importance of Chemistry.

(ii) Properties of matter and their measurement:- Physical and chemical properties, Sl units, mass and weight, volume, density, temperature

(iii) Uncertainty in measurement: -Scientific notation, multiplication and division, addition and subtraction, significant figures, precision and accuracy, dimensional analysis.

(iv) Atomic and molecular Masses-atomic mass, average atomic max, molecular mass, formula mass.

(v) Mole concept and molar masses.

(vi) Percentage Composition:- empirical Formula and melular formula.

(vii) Stoichiometry and calculations:-Balancing of chemical equations, limiting reagent, mais percentage, mole fraction, molarity, molality.

Unit II: Structure of Atom

(i) Sub. atomic particles, charge to mass ratio of electron, charge on the electron.

(ii) Atomic Models: mass mumber, Drawbacks of Rutherford's model.

(iii) Developments leading to the Bohr's model of atom - Wave nature of electromagnetic radiations, electromagnetic spectrum, particle nature of electromagnetic radiation, Planck's quantum theory, photo electric effects. Dual behavior of electromagnetic radiations, atomic spectra, emission and absorption spectrum.

(iv) Bohr's Model for Hydrogen atom: -Explaination of line spectrum of hydrogen Limitations of Bohr's Model.

(v) Quantum mechanical model of the atom:- Dual nature of matters and light, Heisenberg's uncertainty principle, it's significance de-Broglie's relationship, failure of Bohr's model, hydrogen atom and the Schrodinger equation.

(vi) Orbital and quantum numbers- Shapes of atomic s,p,d and f orbitals energies of orbitals rules for filling of electrons in orbitals Aufbau principle pauli exclusion principle and Hund's rule, electronic configuration. of atoms, stability of half filled and full filled orbitals.

Unit III: Classification of Elements and Periodicity in Properties

(i) Need of Classification of elements, basis of periodic Classification, Newlands law of Octaves.

(ii) Electronic configurations and types of elements s,p,d,f - Blocks, metals, non metals and metalloids.

(iii) Periodic trends in properties of elements:- Trends in physical properties, atomic radii, Ionic radii, ionization enthalpy, electron gain enthalpy, electro negativity. 

(iv) Periodic trends in chemical properties:- Periodicity of valence or oxidations states, anamolous properties of second period elements. Periodic trends and chemical reactivity.

Unit IV: Chemical Bonding and Molecular Structure

(i) Kossel - Lewis Approach to chemical bonding:- Octet rule, Covalent Bond, Lewis representation of simple molecules (Lewis structure), Formal Charge Limitation of the octet rule.

(ii) Ionic OR Electrovalent Bond:- Lattice enthalpy.

(iii) Bond Parameters - Bond length, bond angle, bond enthalpy. bond-order, resonance structures, polarity of bonds, dipole moments.

(iv) The Valence Shell Electon Pair Repulsion (VSEPR) Theory.

(v) Valence Bond Theory: Orbital overlap concept, directional properties of bonds, overlapping of atomic orbital, types of overlapping and nature of covalent bond, sigma bond and pi bond.

(vi) Hybridisation-Types of hybridisation and shapes of molecules.

(vii) Molecular orbital theory:- Formation of molecular orbitals Liner combination of atomic orbital (LC

OFFICIAL SYLLABUS

Unit I: Some Basic Concepts of Chemistry

(i) Importance of Chemistry.

(ii) Properties of matter and their measurement:- Physical and chemical properties, Sl units, mass and weight, volume, density, temperature

(iii) Uncertainty in measurement: -Scientific notation, multiplication and division, addition and subtraction, significant figures, precision and accuracy, dimensional analysis.

(iv) Atomic and molecular Masses-atomic mass, average atomic max, molecular mass, formula mass.

(v) Mole concept and molar masses.

(vi) Percentage Composition:- empirical Formula and melular formula.

(vii) Stoichiometry and calculations:-Balancing of chemical equations, limiting reagent, mais percentage, mole fraction, molarity, molality.

Unit II: Structure of Atom

(i) Sub. atomic particles, charge to mass ratio of electron, charge on the electron.

(ii) Atomic Models: mass mumber, Drawbacks of Rutherford's model.

(iii) Developments leading to the Bohr's model of atom - Wave nature of electromagnetic radiations, electromagnetic spectrum, particle nature of electromagnetic radiation, Planck's quantum theory, photo electric effects. Dual behavior of electromagnetic radiations, atomic spectra, emission and absorption spectrum.

(iv) Bohr's Model for Hydrogen atom: -Explaination of line spectrum of hydrogen Limitations of Bohr's Model.

(v) Quantum mechanical model of the atom:- Dual nature of matters and light, Heisenberg's uncertainty principle, it's significance de-Broglie's relationship, failure of Bohr's model, hydrogen atom and the Schrodinger equation.

(vi) Orbital and quantum numbers- Shapes of atomic s,p,d and f orbitals energies of orbitals rules for filling of electrons in orbitals Aufbau principle pauli exclusion principle and Hund's rule, electronic configuration. of atoms, stability of half filled and full filled orbitals.

Unit III: Classification of Elements and Periodicity in Properties

(i) Need of Classification of elements, basis of periodic Classification, Newlands law of Octaves.

(ii) Electronic configurations and types of elements s,p,d,f - Blocks, metals, non metals and metalloids.

(iii) Periodic trends in properties of elements:- Trends in physical properties, atomic radii, Ionic radii, ionization enthalpy, electron gain enthalpy, electro negativity. 

(iv) Periodic trends in chemical properties:- Periodicity of valence or oxidations states, anamolous properties of second period elements. Periodic trends and chemical reactivity.

Unit IV: Chemical Bonding and Molecular Structure

(i) Kossel - Lewis Approach to chemical bonding:- Octet rule, Covalent Bond, Lewis representation of simple molecules (Lewis structure), Formal Charge Limitation of the octet rule.

(ii) Ionic OR Electrovalent Bond:- Lattice enthalpy.

(iii) Bond Parameters - Bond length, bond angle, bond enthalpy. bond-order, resonance structures, polarity of bonds, dipole moments.

(iv) The Valence Shell Electon Pair Repulsion (VSEPR) Theory.

(v) Valence Bond Theory: Orbital overlap concept, directional properties of bonds, overlapping of atomic orbital, types of overlapping and nature of covalent bond, sigma bond and pi bond.

(vi) Hybridisation-Types of hybridisation and shapes of molecules.

(vii) Molecular orbital theory:- Formation of molecular orbitals Liner combination of atomic orbital (LCAO), conditions for the combination of atomic orbital, types of molecular orbitals, energy level diagram for molecular orbitals, electronic configuration and molecular behaviour. Bonding in same homo nuclear diatomic modicules. (qualitative idea only)

(viii) Hydrogen Bonding - Cause of formation of hydrogen bond types of hydrogen bond.

Unit V: States of Matter: Gases and Liquids

(i) Inter molecular forces - Dispersion forces, dipole dipole forces, dipole induced dipole forces, hydrogen bond. 

(ii) Thermal energy.

(iii) Intermolecular forces V/s Thermal interactions.

(iv) The Geseous state -The Gas Laws, Boyle's law, Charle's law, Gay Lussac's law, Avogadro's law.

(v) Ideal gas equation:- density and molar mass of gas, Dalton law of partial pressure, partial pressure in terms of mole fraction.

(vii) Deviation from ideal gas behaviour.

Unit VI: Thermodynamics

(i) Thermodynamic state:- system and surroundings, types of systems, open, closed and isolated system, state function and path functions. Internal energy as a state function, work, beat, isothermal and free expansion of an ideal gas.

(ii) Enthalpy, extensive and intensive properties.

(iii) Calorimetry-Measurement of ?U and ?H, bomb calorimeter.

(iv) Enthalpy Change - reaction enthalpy, standard enthalpy of reactions, enthalpy changes during phase trans formations, standard enthalpy of formation Hess's law of constant heat summation.

(v) Enthalpies for different types of reactions:- Standard enthalpy of combustion, enthalpy of atomization, bond enthalpy, enthalpy of solution, lattice enthalpy.

(vi) Spontaneity- Factors governing spontaneity of process, Change in enthalpy and change in entropy, Gibb's free energy, effect of temp on spontaneity of process, Gibb's free energy change. 

Unit VII: Equilibrium

(i) Equilibrium in physical process Solid- equilibrium, equilibrium involving dissolution of solid or gass in liquids, general characterinics of equilibrium involving physical processes.

(ii) Equilibrium in chemical processes- dynamic equilibrium.

(iii) Law of Chemical equilibrium and equilibrium constant- relation between equilibrium constant for a general reaction and its multiple.

(iv) Homogeneous equilibrium:- relationship between equilibrium constant in terms of pressure(Kp) and equilibrium constant in terms concentration(Kc).

(v) Heterogeneous equilibrium.

(vi) Application of equilibrium constant, predicting the extent of a reaction, predicting the direction of the reaction, calculating equilibrium concentration.

(vii) Relationship between equilibrium constant (K), reaction quotient (Q) and Gibb's energy (G).

(viii) Factors affecting equilibrium: Le Chatelier's principle, effect of changing Concentration, effect of pressure change, effect of temp change, effect of inert Gas addition, effect of catalyst.

(ix) Ionic equilibrium in solutions- acids, bases and salts, Arrhenius concept of acids and bases, Bronsted Lowry acids and bases, Lewis acids and bases.

(x) Ionization of acids and bases.

(xi) Ionization constant of water and its ionic product- pH Scale, lonization of weak acids, ionization of weak bases, relationship between Ka and Kb, di and ply basic acids & strength, Common ion effect, pH of their solution.

(xii) Buffer Solutions.

(xiii) Solubility equilibrium of sparingly soluble salts, solubility product common ion effect on solubility of ionic salts.

Unit VIII: Redox Reactions

(i) Oxidation and reduction reactions.

(ii) Redox reactions in terms of electron transfer reactions.

(iii) Oxidation reactions by oxidactin number method and half reaction method, redox reactions as the basis for titractions.

(iv) Redox reactions and electode processes standard electrode potential.

Unit IX: Hydrogen

(i) Position of hydrogen in the periodic table.

(ii) Dihydrogen- Occurence, isotopes if hydrogen.

(iii) Preparation of dihydrogen.

(iv) Properties of dihydrogen, uses of dihydrogen.

(v) Hydrides Ionic, covalent, Metallic hydndes.

(vi) Water: Physical Properties, Structure of water, Structure of ic, Chemical properties of water, Hard and Soft water, Methods for softening of water.

(vii) Heavy water.

(viii) Dihydrogen as a fuel.

Unit X:  The S-Block Elements (Alkali and Alkaline Earth Metals)

(i) Alkali metals:- Electronic configuration, Atomic and Ionic Radii, Ionization Enthalpy, Hydration Enthalpy, physical properties, chemical properties, uses.

(ii) Compounds of alkali metals:- Oxides and hydroxides, halides, salts of oxoacids.

(iii) Anamolous properties of lithium- diffence between Iithium and other alkali metals similarities between lithium and magnisium.

(iv) Alkaline earth metals:- Electronic configuration, Atomic and Ionic Radii, Ionization enthalpy, Hydration enthalpy, physical and chemical properties, uses.

(v) Compounds of the alkaline earth metals.

(vi) Anamolous behaviour of beryllium, diagonal relationship between beryllium and aluminium.

Unit XI: P-Block Elements

(i) Electronic configuration, atomic radii, ionization enthalpy, electronegativity, physical and chemical properties.

(ii) Anamolous properties of Boron.

(iii) Uses of boron, Aluminium and their compounds.

(iv) Group 14 Elements:- Electronic Configuration, covalent radii, ionization enthalpy, electronegativity, Physical properties, Chemical properties.

(v) Anamolous behaviour of Carbon.

(vi) Allotropes of Carbon- Diamond, graphite, fullerenes uses of carbon.

Unit XII: Organic Chemistry-Some Basic Principles and Techniques

(i) Introduction, shapes of Carbon compounds.

(ii) Complete, Condensed and bond line structural formulas three dimensional representation of organic molecules.

(iii) Classification of organic compounds: Functional groups, hemologous series.

(iv) Nomenclature of Organic Compounds: IUPAC system of nomenclature of organic compounds, nomenclature of substituted benzene compounds.

(v) Isomerism:- structural, stereoisomerism

(vi) Concepts in organic reaction mechanism:- Fission of a covalent bond, nucleophiles and electrophiles, electron movement in organic reactions, inductive effect, resonance structures, resonance effect, electromeric effect, hyperconjugation, types of organic reactions and mechanisms.

(vii) Methods of purification of organic Compounds:-  sublimation, crystallisation, distillation, fractional distillation, steam distillation, differential extraction chromatography.

Unit XIII: Hydrocarbons 

(i) Clasification.

(ii) Alkanes: Nomenclature and isomerism, preparation of alkanes, physical and chemical properties of alkanes, substitution reactions, controlled oxidation, isomerisation, aromatization, confirmations: Sawhorse projections, Newman projections.

(iii) Alkenes: Structure, nomenclature, isomerism, preparation of alkenes, physical properties and chemical properties: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov's addition and peroxide effect) oxidation, ozonolysis, polymerization.

(iv) Alkynes: Nomenclature isomerism, structure of triple bond, methods of preparation, physical properties, chemical reactions:-  acidic character of alkynes, addition reactions of hydrogen, halogens, hydrogen halides, water, polymerization.

(v) Aromatic hydrocarbons Introduction IUPAC nomenclature; Isomerism, Benzene: Physical Properties and chemical paroperties: electrophilic substitution: nitration halogenation, sulphonation, Friedel- Craft's alkylation and acylation, mechanism of electrophilic substitution reaction; deirective influence of functional group in mono substituted benzene; Carcinogenicity and toxicity.

PRACTICAL SYLLABUS

Micro-chemical methods are available for several of the practical experiments. Wherever possible, such techniques should be used.

A. Basic Laboratory Techniques

1. Cutting glass tube and glass rod

2. Bending a glass tube

3. Drawing out a glass jet

4. Boring a cork

B. Characterization and Purification of Chemical Substances

1. Determination of melting point of an organic compound.

2. Determination of boiling point of an organic compound.

3. Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.

C. Experiments releted to pH

a) Any one of the following experiments:

1. Determination of pH of some solutions obtained from fruit juices, solution of known and varied concentrations of acids, bases and salts using pH paper or universal indicator.

2. Comparing the pH of solutions of strong and weak acids of same concentration.

3. Study the pH change by common ion effect in case of weak acid and weak bases.

D. Chemical Equilibrium

One of the following experiments:

1. Study the shift in equilibrium between ferric iron and thiocyanate ions by increasing/decreasing the concentration of either of the ions.

2. Study the shift  in equilibrium between [Co(H₂O)₆]²⁺ and chloride ions by changing the concentration of either of the ions.

E. Quantitative Estimation

1. Using a mechanical balance/electronic balance.

2. Preparation of standard solution of Oxalic acid.

3. Determination of strength of a given solution of Sodium hydroxide by titrating it against standard solution of Oxalic acid.

4. Preparation of standard solution of Sodium carbonate.

5. Determination of strength of a given solution of hydrochloric acid by titrating it against standard Sodium Carbonate solution.

F. Qualitative Analysis

1. Determination of one cation and one anion in a given salt.

Cation : Pb²⁺, Cu²⁺, As³⁺, Al³⁺, Fe³⁺, Mn²⁺, Zn²⁺, Cu²⁺, Ni²⁺, Ca²⁺, Sr²⁺, Ba²⁺, Ng²⁺, NH₄⁺

Anions: (CO₃)^2-, S^2-, (SO₃)^2-, (NO₂)^-, (SO₄)^2-, Cl^-, Br^-, I^-, PO₄^-, C₂O^2-₄, CH₃COO^- 

2. Anyone Project

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